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- Identify the following atoms: (a) It has the ground-state electron configuration [Ar] 4s2 3d10 4p1.
Problem 109
Problem 110a
Write the symbol, give the ground-state electron configuration, and draw an orbital-filling diagram for each of the following atoms. Use the abbreviation of the preceding noble gas to represent the inner-shell electrons. (a) The heaviest alkaline earth metal
Problem 110c
Write the symbol, give the ground-state electron configuration, and draw an orbital-filling diagram for each of the following atoms. Use the abbreviation of the preceding noble gas to represent the inner-shell electrons.
(c) The heaviest actinide metal
- Given the subshells 1s, 2s, 2p, 3s, 3p, and 3d, identify those that meet the following descriptions: (c) Is empty in a nitrogen atom (d) Is full in a carbon atom.
Problem 111
Problem 111a
Given the subshells 1s, 2s, 2p, 3s, 3p and 3d, identify those that meet the following descriptions. (a) Has l = 2
Problem 111b
Given the subshells 1s, 2s, 2p, 3s, 3p and 3d, identify those that meet the following descriptions. (b) Can have ml = -1
Problem 111e
Given the subshells 1s, 2s, 2p, 3s, 3p and 3d, identify those that meet the following descriptions. (e) Contains the outermost electrons in a beryllium atom
Problem 111f
Given the subshells 1s, 2s, 2p, 3s, 3p and 3d, identify those that meet the following descriptions. (f) Can contain two electrons, both with spin ms = +1/2
- Assuming that g orbitals fill according to Hund's rule, what is the atomic number of the first element to have a filled g orbital?
Problem 113
- Cyclooctatetraene dianion, C8H8 2-, is an organic ion with the structure shown. Considering only the p bonds and not the s bonds, cyclooctatetraene dianion can be described by the following energy diagrams of its p molecular orbitals:
Problem 115
(d) Based on your MO energy diagram, is the dianion paramagnetic or diamagnetic?
- What is the expected ground-state electron configuration of the recently discovered element with Z = 116?
Problem 116
- What is the atomic number and expected ground-state electron configuration of the yet undiscovered element directly below Fr in the periodic table?
Problem 117
- Why do atomic radii increase going down a group of the periodic table?
Problem 118
Problem 119
Why do atomic radii decrease from left to right across a period of the periodic table?
- Fill in the blanks with the appropriate region of electromagnetic radiation: UV, visible, infrared. (a) The Sun most strongly emits in the _____ and regions of electromagnetic radiation (b) The atmosphere filters out biologically damaging ______ radiation from incoming solar radiation and prevents it from reaching Earth. (c) The Earth most strongly emits ______ radiation. (d) Greenhouse gases absorb _______ radiation.
Problem 120
Problem 121
Order the following atoms according to increasing atomic radius: Rb, Cl, As, K.
- Why do the Earth and Sun have different emission spectra?
Problem 122
- Orbital energies in single-electron atoms or ions, such as He+, can be described with an equation similar to the Balmer–Rydberg equation:
Problem 124
where Z is the atomic number. What wavelength of light in nanometers is emitted when the electron in He+ falls from n = 3 to n = 2?
Problem 126a
Imagine a universe in which the four quantum numbers can have the same possible values as in our universe except that the angular-momentum quantum number l can have integral values of 0, 1, 2...n + 1 (instead of 0, 1, 2..., n - 1). (a) How many elements would be in the first two rows of the periodic table in this universe?
- One watt (W) is equal to 1 J/s. Assuming that 5.0% of the energy output of a 75 W light bulb is visible light and that the average wavelength of the light is 550 nm, how many photons are emitted by the light bulb each second?
Problem 130
- Microwave ovens work by irradiating food with microwave radiation, which is absorbed and converted into heat. Assum-ing that radiation with l = 15.0 cm is used, that all the energy is converted to heat, and that 4.184 J is needed to raise the temperature of 1.00 g of water by 1.00 °C, how many photons are necessary to raise the temperature of a 350 mL cup of water from 20 °C to 95 °C?
Problem 131
- The amount of energy necessary to remove an electron from an atom is a quantity called the ionization energy, Ei. This energy can be measured by a technique called photoelectron spectroscopy, in which light of wavelength l is directed at an atom, causing an electron to be ejected. The kinetic energy of the ejected electron (Ek) is measured by determining its veloc-ity, v (Ek = mv2/2), and Ei is then calculated using the conservation of energy principle. That is, the energy of the incident light equals Ei plus Ek. What is the ionization energy of selenium atoms in kilojoules per mole if light with l = 48.2 nm produces electrons with a velocity of 2.371 * 106 m/s? The mass, m, of an electron is 9.109 * 10-31 kg.
Problem 132
- X rays with a wavelength of 1.54 * 10-10 m are produced when a copper metal target is bombarded with high-energy electrons that have been accelerated by a voltage difference of 30,000 V. The kinetic energy of the electrons equals the product of the voltage difference and the electronic charge in coulombs, where 1 volt-coulomb = 1 J. (a) What is the kinetic energy in joules and the de Broglie wavelength in meters of an electron that has been accel-erated by a voltage difference of 30,000 V?
Problem 133
- In the Bohr model of atomic structure, electrons are constrained to orbit a nucleus at specific distances, given by the equation
Problem 134
where r is the radius of the orbit, Z is the charge on the nucleus, a0 is the Bohr radius and has a value of 5.292 * 10-11 m, and n is a positive integer (n = 1, 2, 3...) like a principal quantum number. Furthermore, Bohr concluded that the energy level E of an electron in a given orbit is
where e is the charge on an electron. Derive an equation that will let you calculate the difference ∆E between any two energy levels. What relation does your equation have to the Balmer–Rydberg equation?
- Assume that the rules for quantum numbers are different and that the spin quantum number ms can have any of three values, ms = -1/2, 0, +1/2, while all other rules remain the same. (a) Draw an orbital-filling diagram for the element with Z = 25, showing the individual electrons in the outer-most subshell as up arrows, down arrows, or 0. How many partially filled orbitals does the element have?
Problem 135
Problem 136a
A minimum energy of 7.21⨉10-19 J is required to produce the photoelectric effect in chromium metal. (a) What is the minimum frequency of light needed to remove an electron from chromium?
Problem 136b
A minimum energy of 7.21⨉10-19 J is required to produce the photoelectric effect in chromium metal. (b) Light with a wavelength of 2.50⨉10-7 m falls on a piece of chromium in an evacuated glass tube. What is the minimum de Broglie wavelength of the emitted electrons? (Note that the energy of the incident light must be conserved; that is, the photon's energy must equal the sum of the energy needed to eject the electron plus the kinetic energy of the electron.)
- (c) What is the velocity of an electron with a de Broglie wavelength equal to (b)?
Problem 137
Problem 138c
An energetically excited hydrogen atom has its electron in a 5f subshell. The electron drops down to the 3d subshell, releasing a photon in the process. (c) The hydrogen atom now has a single electron in the 3d subshell. What is the energy in kJ/mol required to remove this electron?
Problem 139a
Consider the noble gas xenon. (a) Write the electron configuration of xenon using the abbreviation of the previous noble gas.